Write a hybridization and bonding scheme for each molecule or ion. Sketch the structure, including overlapping orbitals, and label all bonds using the notation shown in Examples 10.6 and 10.7. a. SO₃^2-

Key Concepts

Hybridization

Hybridization is the process of mixing atomic orbitals to form new hybrid orbitals that are suitable for the pairing of electrons to form chemical bonds. In the case of the sulfate ion (SO3^2-), the central sulfur atom undergoes hybridization to accommodate the bonding with oxygen atoms, typically resulting in sp3 hybridization due to the tetrahedral arrangement of electron pairs.

Bonding and Molecular Geometry

Bonding refers to the interactions between atoms that lead to the formation of molecules or ions. The molecular geometry of SO3^2- is determined by the arrangement of its bonded atoms and lone pairs around the central sulfur atom, which can be predicted using the VSEPR (Valence Shell Electron Pair Repulsion) theory. This results in a trigonal pyramidal shape due to the presence of one lone pair.

Orbital Overlap and Bonding Notation

Orbital overlap is a key concept in understanding how atoms bond together, as it describes the interaction between atomic orbitals of different atoms that leads to the formation of covalent bonds. In the bonding scheme for SO3^2-, it is important to illustrate the overlapping orbitals between sulfur and oxygen atoms, and to label the bonds (single, double) using appropriate notation to indicate the type and strength of the bonds formed.